QBManager

Ionic Equilibrium

229609 The acid present in vinegar is

1

{CH}_{3} COOH

2

H_{2} {SO}_{4}

3

HCl

4

{HNO}_{3}

Explanation:

Vinegar is a liquid consisting mainly of acetic acid $({CH}_{3} COOH)$ and water. The acetic acid is produced by the fermentation of ethanol by acetic acid bacteria.
Vinegar is now mainly used as a cooking ingredient.

CG PET-2004

Ionic Equilibrium

229611 The $pH$ of water decreases with?

1 Increase in temperature

2 Increase in pressure

3 Decrease in temperature

4 Decrease in pressure

Explanation:

An Increase in temperature increases $K_{π}$ and a decreases in temperature decreases $K_{i}$ .
The neutral $pH$ point depends on the $K_{π}$ of water where both $H$ and $OH$ ion are equal in number. Hence, $pH$ of water decreases with increase in temperature.

CG PET-2005

Ionic Equilibrium

229612 The aqueous solution of which one of the following is basic?

1

HOCl

2

{NaHSO}_{4}

3

{NH}_{4} {NO}_{3}

4

NaOCl

Explanation:

The mixture of strong base and weak acid is basic solution.
Hence, $NaOCl$ is a mixture of strong base and weak acid. So, aqueous solution is basic.

CG PET-2005

Ionic Equilibrium

229527 Which of the following can act both as Bronsted acid and Bronsted base?
(i) ${HCO}_{3}^{-}$ (ii) ${NH}_{3}$ (iii) $O^{2 -}$ (iv) $HCl$

1 (i) and (ii)

2 (ii) and (iii)

3 None of the above

4 All of the above

Explanation:

Those substance which accept the proton are called Bronsted base and which is donate the proton are called Bronsted acid.
${HCO}_{3}^{-} + H^{+} = H_{2} {CO}_{3}$ Bronsted base.
${HCO}_{3}^{-} = H^{+} + {CO}_{3}^{2 -}$ Bronsted acid.

AP-EAMCET-1995

Ionic Equilibrium

229609 The acid present in vinegar is

1

{CH}_{3} COOH

2

H_{2} {SO}_{4}

3

HCl

4

{HNO}_{3}

Explanation:

Vinegar is a liquid consisting mainly of acetic acid $({CH}_{3} COOH)$ and water. The acetic acid is produced by the fermentation of ethanol by acetic acid bacteria.
Vinegar is now mainly used as a cooking ingredient.

CG PET-2004

Ionic Equilibrium

229611 The $pH$ of water decreases with?

1 Increase in temperature

2 Increase in pressure

3 Decrease in temperature

4 Decrease in pressure

Explanation:

An Increase in temperature increases $K_{π}$ and a decreases in temperature decreases $K_{i}$ .
The neutral $pH$ point depends on the $K_{π}$ of water where both $H$ and $OH$ ion are equal in number. Hence, $pH$ of water decreases with increase in temperature.

CG PET-2005

Ionic Equilibrium

229612 The aqueous solution of which one of the following is basic?

1

HOCl

2

{NaHSO}_{4}

3

{NH}_{4} {NO}_{3}

4

NaOCl

Explanation:

The mixture of strong base and weak acid is basic solution.
Hence, $NaOCl$ is a mixture of strong base and weak acid. So, aqueous solution is basic.

CG PET-2005

Ionic Equilibrium

229527 Which of the following can act both as Bronsted acid and Bronsted base?
(i) ${HCO}_{3}^{-}$ (ii) ${NH}_{3}$ (iii) $O^{2 -}$ (iv) $HCl$

1 (i) and (ii)

2 (ii) and (iii)

3 None of the above

4 All of the above

Explanation:

Those substance which accept the proton are called Bronsted base and which is donate the proton are called Bronsted acid.
${HCO}_{3}^{-} + H^{+} = H_{2} {CO}_{3}$ Bronsted base.
${HCO}_{3}^{-} = H^{+} + {CO}_{3}^{2 -}$ Bronsted acid.

AP-EAMCET-1995

Ionic Equilibrium

229609 The acid present in vinegar is

1

{CH}_{3} COOH

2

H_{2} {SO}_{4}

3

HCl

4

{HNO}_{3}

Explanation:

Vinegar is a liquid consisting mainly of acetic acid $({CH}_{3} COOH)$ and water. The acetic acid is produced by the fermentation of ethanol by acetic acid bacteria.
Vinegar is now mainly used as a cooking ingredient.

CG PET-2004

Ionic Equilibrium

229611 The $pH$ of water decreases with?

1 Increase in temperature

2 Increase in pressure

3 Decrease in temperature

4 Decrease in pressure

Explanation:

An Increase in temperature increases $K_{π}$ and a decreases in temperature decreases $K_{i}$ .
The neutral $pH$ point depends on the $K_{π}$ of water where both $H$ and $OH$ ion are equal in number. Hence, $pH$ of water decreases with increase in temperature.

CG PET-2005

Ionic Equilibrium

229612 The aqueous solution of which one of the following is basic?

1

HOCl

2

{NaHSO}_{4}

3

{NH}_{4} {NO}_{3}

4

NaOCl

Explanation:

The mixture of strong base and weak acid is basic solution.
Hence, $NaOCl$ is a mixture of strong base and weak acid. So, aqueous solution is basic.

CG PET-2005

Ionic Equilibrium

229527 Which of the following can act both as Bronsted acid and Bronsted base?
(i) ${HCO}_{3}^{-}$ (ii) ${NH}_{3}$ (iii) $O^{2 -}$ (iv) $HCl$

1 (i) and (ii)

2 (ii) and (iii)

3 None of the above

4 All of the above

Explanation:

Those substance which accept the proton are called Bronsted base and which is donate the proton are called Bronsted acid.
${HCO}_{3}^{-} + H^{+} = H_{2} {CO}_{3}$ Bronsted base.
${HCO}_{3}^{-} = H^{+} + {CO}_{3}^{2 -}$ Bronsted acid.

AP-EAMCET-1995

Ionic Equilibrium

229609 The acid present in vinegar is

1

{CH}_{3} COOH

2

H_{2} {SO}_{4}

3

HCl

4

{HNO}_{3}

Explanation:

Vinegar is a liquid consisting mainly of acetic acid $({CH}_{3} COOH)$ and water. The acetic acid is produced by the fermentation of ethanol by acetic acid bacteria.
Vinegar is now mainly used as a cooking ingredient.

CG PET-2004

Ionic Equilibrium

229611 The $pH$ of water decreases with?

1 Increase in temperature

2 Increase in pressure

3 Decrease in temperature

4 Decrease in pressure

Explanation:

An Increase in temperature increases $K_{π}$ and a decreases in temperature decreases $K_{i}$ .
The neutral $pH$ point depends on the $K_{π}$ of water where both $H$ and $OH$ ion are equal in number. Hence, $pH$ of water decreases with increase in temperature.

CG PET-2005

Ionic Equilibrium

229612 The aqueous solution of which one of the following is basic?

1

HOCl

2

{NaHSO}_{4}

3

{NH}_{4} {NO}_{3}

4

NaOCl

Explanation:

The mixture of strong base and weak acid is basic solution.
Hence, $NaOCl$ is a mixture of strong base and weak acid. So, aqueous solution is basic.

CG PET-2005

Ionic Equilibrium

229527 Which of the following can act both as Bronsted acid and Bronsted base?
(i) ${HCO}_{3}^{-}$ (ii) ${NH}_{3}$ (iii) $O^{2 -}$ (iv) $HCl$

1 (i) and (ii)

2 (ii) and (iii)

3 None of the above

4 All of the above

Explanation:

Those substance which accept the proton are called Bronsted base and which is donate the proton are called Bronsted acid.
${HCO}_{3}^{-} + H^{+} = H_{2} {CO}_{3}$ Bronsted base.
${HCO}_{3}^{-} = H^{+} + {CO}_{3}^{2 -}$ Bronsted acid.

AP-EAMCET-1995

Question Bank Series

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